Question

Barium chloride has the formula BaCl2. x H2O. On heating 4.88g of barium chloride crystals, 4.16g of anhydrous barium chloride remain. Calculate the value of x in BaCl2. x H2O.

Answer 1

Answer on Question #45208, Chemistry, Inorganic Chemistry

Question

Barium chloride has the formula BaCl₂. x H₂O. On heating 4.88g of barium chloride crystals, 4.16g of anhydrous barium chloride remain. Calculate the value of x in BaCl₂. x H₂O.

Solution

4.16g of anhydrous barium chloride is related to:

$$n(\mathrm{BaCl_2}) = \mathrm{m/M} = 4.16 / 208,23 = 0.02 \text{ mole}.$$

4.88g – 4.16g = 0.72g is the mass of H₂O in BaCl₂ x H₂O. Thus:

$$n(\mathrm{H_2O}) = \mathrm{m/M} = 0.72 / 18.015 = 0.04 \text{ mole}.$$

$n(\mathrm{H_2O}) = 2 n(\mathrm{BaCl_2})$ therefore the formula is $\mathrm{BaCl_2 \cdot 2H_2O}$, $x = 2$.

Answer: $x = 2$

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